(a)
Interpretation:
The MO diagram, the number of unpaired electrons, the number bonds in
Concept Introduction:
Molecular orbital theory:
The atomic orbitals of the atoms constituted in a molecule are combined to produce new orbitals are called Molecular Orbitals.
Like atomic orbitals, a molecular orbital can accommodate maximum two electrons and the two electrons must have opposite spins (Pauli Exclusion Principle).
The numbers of MO’s are equals to the number of atomic orbitals are combined in such a way that the linear combination of similar atomic orbitals to form one bonding and one anti-bonding MO’s.
The bonding MO’s are lower in energy than the anti-bonding MO’s.
HOMO is the highest energized occupied orbital in the MO’s.
Relative energy levels of molecules are according to the energy levels of atomic orbitals.
LUMO is the lowest energized orbital in the MO’s.
Bond order can be calculated using below formula
(a)
Explanation of Solution
The total number of valence electrons present in
The molecular orbital diagrams of the
The bond order can be calculated using bonding and anti-bonding orbitals, the bond order is
Therefore, the
(b)
Interpretation:
The MO diagram, the number of unpaired electrons, the number bonds in
Concept Introduction:
Refer part (a).
(b)
Explanation of Solution
The total number of valence electrons present in
The molecular orbital diagrams of the
The bond order can be calculated using bonding and anti-bonding orbitals, the bond order is
Therefore, the
(c)
Interpretation:
The MO diagram, the number of unpaired electrons, the number bonds in
Concept Introduction:
Refer part (a).
(c)
Explanation of Solution
The total number of valence electrons present in
The molecular orbital diagrams of the
The bond order can be calculated using bonding and anti-bonding orbitals, the bond order is
Therefore, the
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Chapter 6 Solutions
OWLV2 FOR MOORE/STANITSKI'S CHEMISTRY:
- Draw the molecular orbital energy diagrams for the valence electrons in the following diatomic molecules. Calculate the bond order and indicate if each of them is diamagnetic or paramagnetic. (а) В> (b) С. (c) CO (d) NO (е) Оzarrow_forwardSiCl, is used as a starting material in the production of silicon polymers. Describe hybridization schemes for the central atom and the orbital overlap that occur in this halogen compound. ( Si, #Cl) 14 Data for the arrangement of electron pairs about a central atom in a molecule and geometry of the molecule and the shape of hybrid orbitals Number of Molecular Number of hybrid Hybridization of electron pairs geometry orbitals the central atom Linear 2 sp Trigonal planar 3 sp 4 Tetrahedral 4 sp 5 Trigonal 5 sp'd bipyramidal Octahedral 6. sp'd 2. 3.arrow_forwardDescribe the molecular geometry and hybridization of the N, P, or S atoms in each of the following compounds. (a) H3PO4, phosphoric acid, used in cola soft drinks (b) NH4NO3, ammonium nitrate, a fertilizer and explosive (c) S2Cl2, disulfur dichloride, used in vulcanizing rubber (d) K4[O3POPO3], potassium pyrophosphate, an ingredient in some toothpastesarrow_forward
- Describe the molecular geometry and hybridization of the N, P, or S atoms in each of the following compounds.(a) H3PO4, phosphoric acid, used in cola soft drinks(b) NH4NO3, ammonium nitrate, a fertilizer and explosive(c) S2Cl2, disulfur dichloride, used in vulcanizing rubber(d) K4[O3POPO3], potassium pyrophosphate, an ingredient in some toothpastesarrow_forwardUsing molecular orbital theory, determine the electronic structure of the first excited electronic state of N2. What differences are expected in the properties of the excited state of N2 compared with the same properties of the ground state?arrow_forwardDraw the best Lewis dot structure for BrCl₅, being sure to give the electronic geometry, molecular geometry, hybridization of the central element, polarity, and bond angle around the cental element.arrow_forward
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- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning